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2 years ago

20 ML of a gas at 200 K is heated until the new volume is 55ML what is the final temperature of the gas

Chemistry

1 answer:

MrRa [10]2 years ago

8 0

Answer:

T2 = 550K

Explanation:

From Charles law;

V1/T1 = V2/T2

Where;

V1 is initial volume

V2 is final volume

T1 is initial temperature

T2 is final temperature

We are given;

V1 = 20 mL

V2 = 55 mL

T1 = 200 K

Thus from V1/T1 = V2/T2, making T2 the subject;

T2 = (V2 × T1)/V1

T2 = (55 × 200)/20

T2 = 550K

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If the heat of fusion for water is 334 j/g, how many Jules are needed to melt 45.0 g of ice at 0.0°c?

finlep [7]

Given parameters:

Heat of fusion of water = 334j/g

Mass of ice = 45g

Temperature of ice = 0.0°c

Unknown:

Amount of heat needed to melt = ?

Solution:

This is simply a phase change and a latent heat is required in this process.

To solve this problem; use the mathematical expression below;

H = mL

where m is the mass

L is the heat of fusion of water;

H = 45 x 334 = 15030J

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3 years ago

Zinc reacts with hydrochloric acid according to the reaction equation Zn ( s ) + 2 HCl ( aq ) ⟶ ZnCl 2 ( aq ) + H 2 ( g ) How ma

REY [17]

Answer:

34.7mL

Explanation:

First we have to convert our grams of Zinc to moles of zinc so we can relate that number to our chemical equation.

So: 6.25g Zn x (1 mol / 65.39 g) = 0.0956 mol Zn

All that was done above was multiplying the grams of zinc by the reciprocal of zincs molar mass so our units would cancel and leave us with moles of zinc.

So now we need to go to HCl!

To do that we multiply by the molar coefficients in the chemical equation:

$\frac{0.0956g Zn}{1 } (\frac{2 mol HCl}{1molZn})$

This leaves us with 2(0.0956) = 0.1912 mol HCl

Now we use the relationship M= moles / volume , to calculate our volume

Rearranging we get that V = moles / M

Now we plug in: V = 0.1912 mol HCl / 5.50 M HCl

V= 0.0347 L

To change this to milliliters we multiply by 1000 so:

34.7 mL

7 0

3 years ago

Natural gas is stored in a spherical tank at a temperature of 13°C. At a given initial time, the pressure in the tank is 117 kPa

drek231 [11]

Answer:

1. the absolute pressure in the tank before filling = 217 kPa

2. the absolute pressure in the tank after filling = 312 kPa

3. the ratio of the mass after filling M2 to that before filling M1 = 1.44

The correct relation is option c ( $\frac{M_{2} }{M_{1} } = \frac{P_{2} T_{1} }{P_{1} T_{2} }$ )

Explanation:

To find -

1. What is the absolute pressure in the tank before filling?

2. What is the absolute pressure in the tank after filling?

3. What is the ratio of the mass after filling M2 to that before filling M1 for this situation?

As we know that ,

Absolute pressure = Atmospheric pressure + Gage pressure

So,

Before filling the tank :

Given - Atmospheric pressure = 100 kPa , Gage pressure = 117 kPa

⇒Absolute pressure ( p1 ) = 100 + 117 = 217 kPa

Now,

After filling the tank :

Given - Atmospheric pressure = 100 kPa , Gage pressure = 212 kPa

⇒Absolute pressure (p2) = 100 + 212= 312 kPa

Now,

As given, volume is the same before and after filling,

i.e. $V_{1}$ = $V_{2}$

As we know that, P ∝ M

⇒ $\frac{p_{1} }{p_{2} } = \frac{m_{1} }{m_{2} }$

⇒ $\frac{m_{2} }{m_{1} } = \frac{p_{2} }{p_{1} }$

⇒ $\frac{m_{2} }{m_{1} } = \frac{312 }{217 } = 1.4378$ ≈ 1.44

Now, as we know that PV = nRT

As V is constant

⇒ P ∝ MT

⇒ $\frac{P}{T}$ ∝ M

⇒ $\frac{M_{2} }{M_{1} } = \frac{P_{2} T_{1} }{P_{1} T_{2} }$

So, The correct relation is c option.

6 0

3 years ago

Abbreviated electron configuration for tellurium

Zinaida [17]

Answer:

The ground state electron configuration of ground state gaseous neutral tellurium is [Kr]. 4d10.

4 0

2 years ago

You have to prepare 100.0 mL of a 0.100 M solution of sodium carbonate. You have a concentrated solution of sodium carbonate tha

Georgia [21]

Answer:

6.9 ml of concentrate

Explanation:

100 ml of .1 M will require .01 moles

from a 1.45 M solution, .01 mole would be

.01 mole / ( 1.45 mole / liter) = 6.9 ml of the concentrate then dilute to 100 ml

4 0

2 years ago